2.26 g of liquid water at 23.5 ◦C was com - pletely converted to ice at 0 ◦C. How much heat was (absorbed/released) by the system during this process?

Givens

m = 2.26 g

c = 4.19 J / (g * oC)

Δt = 23.5oC - 0 = 23.5oC

hf = heat of fusion for ice = 334 J/g

Equation

H = m*c*Δt + hf * m

H = m * (c*Δt + hf)

Solution

H = 2.26 * (4.19 * 23.5 + 334)

H = 2.26 * (432.5)

H = 977.4 J